Self-clinkering burning rate modifier for solid propellant NF3 -F.sub.2

ABSTRACT

N 2  F 3  SnF 5  is formed by reacting N 2  F 3  SbF 6  and Cs 2  SnF 6  in the presence of HF. N 2  F 3  SnF 5  is useful as a component of NF 3  -F 2  gas generating compositions.

BACKGROUND OF THE INVENTION

1. Field of the Invention

This invention relates to a composition of matter which is useful in NF₃ -F₂ gas generator formulations.

2. Description of the Prior Art

In the recent past, certain new self-clinkering NF₄ ⁺ salts have been synthesized. Among these are (NF₄)₂ SnF₆, NF₄ SnF₅, (NF₄)₂ TiF₆, NF₄ TiF₉, NF₄ Ti₃ F₁₃, NF₄ Ti₆ F₂₅ and (NF₄)₂ NiF₆. When such self-clinkering salts are utilized as oxidizers and combined with a fuel such as aluminum, NF₃ gas, F₂ gas and solids are produced when the combination is burned. The gases are useful as lasing materials. The fact that solids or "clinkers" are produced is important in that it overcomes a disadvantage present when, for example NF₄ BF₄ is used as the oxidizer. When NF₄ BF₄ is used, NF₃, F₂ and another gas, BF₃, are produced. The gaseous BF₃ is not useful as a laser material and acts to deactivate the laser. By producing a solid or "clinker" instead of gases other than NF₃ and F₂, the self-clinkering salts overcome this problem.

Frequently, formulations containing NF₄ ⁺ salts require burning rate modifiers. Typically, N₂ F₃ ⁺ salts which are more reactive than NF₄ ⁺ salts can be used. However, insofar as is known from the prior art, no self-clinkering N₂ F₃ ⁺ salts are available.

SUMMARY OF THE INVENTION

According to this invention, a self-clinkering N₂ F₃ ⁺ salt which is useful as a burning rate modifier has been prepared. The salt has the formula N₂ F₃ SnF₅. Synthesis is accomplished by means of a reaction between N₂ F₃ SbF₆ and Cs₂ SnF₆ in HF. Insofar as is known by the inventors, the salt of this invention is the first self-clinkering N₂ F₃ ⁺ salt ever produced.

DESCRIPTION OF THE PREFERRED EMBODIMENT

The salt, N₂ F₃ SbF₆, may be prepared according to the procedure set forth in the following example

EXAMPLE I

Synthesis of N₂ F₃ SbF₆. A Teflon amplule, containing a Teflon coated magnetic stirring bar and equipped with a stainless steel valve, was loaded with 14.4 mmol of SbF₅ in a glovebox. The ampule was then attached to a vacuum line and 2 ml of anhydrous HF was condensed into the ampule at -78° C. while stirring and warming to ambient temperature. The system was then pressurized with N₂ F₄ (1 atm). A gradual decrease in the pressure was noted due to uptake of N₂ F₄. Periodic cycling to below 0° C. seemed to increase the rate of N₂ F₄ uptake. After several hours the unreacted N₂ F₄ and HF solvent were pumped off at 40° C. until constant weight was achieved. The observed weight gain corresponded to the reaction of 12.1 mmol of N₂ F₄. When the reaction was repeated on a larger scale with 8 ml HF for 3 days, it was found that 74.0 mmol of SbF₅ reacted with 73.5 mmol of N₂ F₄ to give 23.66 g of N₂ F₃ SbF₆ (weight calcd for 74.0 mmol of N₂ F₃ SbF₆ 23.74 g), which was characterized by ¹⁹ F NMR and vibrational spectroscopy.

To produce the salt of this invention, N₂ F₃ SnF₅, one utilizes N₂ F₃ SbF₆ obtained from Example 1 and Cs₂ SnF₆ and carries out the procedure set forth in the following example.

EXAMPLE II

Solid N₂ F₃ SbF₆ (6.43 mmol) and Cs₂ SnF₆ (3.24 mmol) were placed in a well passivated (with CIF₃) Monel vacuum line equipped with Teflon-FEP U traps and diaphragm values. Approximately 2 ml of anhyrous HF was added. After stirring and shaking vigorously for 30 minutes at room temperature, some of the HF was removed under vacuum and the mixture was cooled to -78° C. The solid and liquid phases were separated by pressure filtration and the volatile products were removed by pumping at 25° C. for 15 hours. The volatile material was separated by fractional consideration and consisted of the HF solvent and N₂ F₄ (3.2 mmol). The filtrate residue (0.3 g) was analyzed by means of vibrational and NMR spectroscopy and shown to be N₂ F₃ SnF₅.

When N₂ F₃ SnF₅ is combined with a fuel such as aluminum and burned NF₃ gas, F₂ gas, N₂ gas and a solid are obtained. (Since N₂ is normally used as an inert diluent its formation does not degrade the performance of a laser.) Thus N₂ F₃ SnF₅ is self-clinkering. That is, a non-gaseous product (the solid or "clinker") rather than a gaseous product (such as the BF₃ produced when NF₄ BF₄ is burned) results upon burning of N₂ F₃ SnF₅. In addition, the useful gases NF₃ and F₂ (and N₂) are produced. Insofar as is known by the inventors, N₂ F₃ SnF₅ is the only self-clinkering N₂ F₃ ⁺ salt that has ever been produced to date. 

What is claimed is:
 1. N₂ F₃ SnF₅.
 2. A method for preparing N₂ F₃ SnF₅ comprising the steps of:forming a solution of N₂ F₃ SbF₆ salt and Cs₂ SnF₆ salt in HF; allowing the salts to react. 